At a certain temperature, the equilibrium constant for the reaction CO2lg) + H2(g) is K. = 2.23. If 2.00 mol of CO, and 2.00 mol of H2 are placed in a 2.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide? COg) + H20(g) %3D 0.810 M 0.599 M 0.511M 0.751M 0.631 M

At a certain temperature, the equilibrium constant for the reaction CO2lg) + H2(g) is K. = 2.23. If 2.00 mol of CO, and 2.00 mol of H2 are placed in a 2.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide? COg) + H20(g) %3D 0.810 M 0.599 M 0.511M 0.751M 0.631 M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given 0.50 mol of NOCI is placed in a one-liter reaction vessel at 700 K and after the system comes to equilibrium the concentration of NOCI became 0.440 M. What is the equilibrium constant? Given the reaction as: 2NOCI(g) → 2NO(g) +Cl2(g) 5.6 x 10-4 2.0 x 10-3 4.1 x 10-3 6.1 x 10-3 8.2 x 10-3
The equilibrium constant, K, for the following reaction is 9.23×10-3 at 304 K. NH4HS(s) =NH3(g) + H2S(g) An equilibrium mixture in a 18.5 L container at 304 K contains 0.268 mol NH4HS(s), 0.133 M NH3 and 6.94×10-2 M H2S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.86 L? [NH3] = [H2S] = ΣΣ
A student ran the following reaction in the laboratory at 282 K: 2NO(g) + Br2(g) = 2NOBr(g) When she introduced 0.170 moles of NO(g) and 0.137 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.135 M. Calculate the equilibrium constant, K., she obtained for this reaction. K.
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) – PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.1997 mol sample of PCl, (g) is injected into an empty 2.40 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCl,] = M [PCl,] = M
Phosphorus pentachloride decomposes according to the chemical equation. PCI5 (g) PCI 3 (g) + Cl 2 ( g) Kc = 1.80 at 25 0 C. A 0. 3200 mol sample of PCI 5 (g) is injected into an empty 3.8 L reaction vessel held at 2 5 0 C. Calculate the concentrations of PCI 5 (g ) and PC| 3 (g) at equilibrium.
For the following reaction 6.0 moles of H₂ were combined with 4.5 moles of Cl₂. The reaction was allowed to proceed in a 1.5 L vessel. At equilibrium there were 3.0 moles of H₂ in the system. Determine the equilibrium concentrations for Cl₂ and HCI. 2HCI H₂ + Cl₂ 1b) Determine the % reaction and decide whether this reaction favours the products or reactants.
The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5, 0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L? [PCl5] = M [PCl3] = M [Cl2] = M
Hydrogen gas and bromine gas are mixed in a sealed container at 250°C and allowed to reach equilibrium. H2(g) + Br2(g) = 2HB1(g) The equilibrium constant for this reaction at 250°C is 65.5. At equilibrium, the concentration of H2 is 0.0510 mol L*1 and the concentration of Brris 0.174 mol L-1 at 250°C. (i) Write the equilibrium constant expression for the above reaction. (ii) Calculate the concentration of HBr in the equilibrium mixture at 250°C (iii) Explain what happens to the concentration of HBr you calculated in (ii) above if the pressure of the equilibrium mixture is increased.
4. For the equilibrium CH₂(g) + 2H₂S(g) = CS₂(g) + 4H₂(g), the concentrations at equilibrium are [CH4] = 0.0804 M, [H₂S] = 0.0608 M, [CS₂] = 0.0196 M, and [H₂] = 0.0784 M at 1400.0 K. Using the equilibrium constant expression from before, calculate Kc.
Consider the following equilibrium system at 355 K. 2NOBr(g) -----> 2NO(g)+Br2(g). If an equilibrium mixture of the three gases at 355 K contains 3.21x10^-2 M NOBr, 2.01x10^-2 M NO,and 3.98x10^-2 M Br2 what is the value of the equilibrium constant K
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.1952 mol sample of PCl, (g) is injected into an empty 2.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI,] = M [PCI,] = M
Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium. The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M. CH4(g) + 2H2S(g) ↔ CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.